Answer:
The percent yield of this reaction is 84.8 % (option A is correct)
Explanation:
Step 1: Data given
The student isolated 15.6 grams of the product = the actual yield
She calculated the reaction should have produced 18.4 grams of product = the theoretical yield = 18.4 grams
Step 2: Calculate the percent yield
Percent yield = (actual yield / theoretical yield ) * 100 %
Percent yield = (15.6 grams / 18.4 grams ) * 100 %
Percent yield = 84.8 %
The percent yield of this reaction is 84.8 % (option A is correct)
Answer:
The answer to your question is below
Explanation:
Data
Aqueous sodium carbonate = Na₂CO₃ (aq)
Aqueous strontium chloride = SrCl₂ (aq)
Solid strontium carbonate = SrCO₃ (s)
Aqueous sodium chloride = NaCl (aq)
Unbalnced Chemical reaction
Na₂CO₃(aq) + SrCl₂(aq) ⇒ SrCO₃(s) + NaCl(aq)
Reactants Elements Products
2 Sodium 1
1 Carbon 1
1 Strontium 1
2 Chlorine 1
3 Oxygen 3
Balanced Chemical reaction
Na₂CO₃(aq) + SrCl₂(aq) ⇒ SrCO₃(s) + 2NaCl(aq)
Reactants Elements Products
2 Sodium 2
1 Carbon 1
1 Strontium 1
2 Chlorine 2
3 Oxygen 3
Answer: It depends equilibrium constant K
Explanation: You need to to have reaction formula.
If K >> 1 then concentrations of products are much bigger than
concentrations of reactants. If K < < 1, concentration of products is small.
Atoms of metals tend to 2. Lose electrons and form positive ions.